Calculate pH of a solution that has [H+] of 6.31 x 10-6 MGroup of answer choices6.36.05.24.7

1. Break Down the Problem

To calculate the pH of a solution, we need to understand that pH is defined as the negative logarithm (base 10) of the hydrogen ion concentration $[H^+]$. The formula to calculate pH is:

$\text{pH} = -\log_{10}([H^+])$

2. Relevant Concepts

In this case, we will use the hydrogen ion concentration given:

$[H^+] = 6.31 \times 10^{-6} \, M$

3. Analysis and Detail

Now we will apply the formula to find the pH:

1. Substitute the value of $[H^+]$ into the pH formula:

$\text{pH} = -\log_{10}(6.31 \times 10^{-6})$

2. Use a calculator to find $-\log_{10}(6.31 \times 10^{-6})$:

• First, calculate the logarithm:

$\log_{10}(6.31) \approx 0.800 \quad \text{(using a calculator)}$

• Then, since it's multiplied by $10^{-6}$, we subtract 6:

$\log_{10}(6.31 \times 10^{-6}) = \log_{10}(6.31) + \log_{10}(10^{-6}) = 0.800 - 6 = -5.200$

3. Therefore:

$\text{pH} = -(-5.200) = 5.200$

4. Verify and Summarize

The calculations show that the pH of the solution, given the hydrogen ion concentration, is approximately 5.20.

Final Answer

$\text{pH} \approx 5.20$

Thus, the correct choice from the options provided is 5.2.